This document discusses different types of intermolecular forces of attraction that hold molecules together, including ion-dipole interactions, London dispersion forces, dipole-dipole forces, hydrogen bonding, and surface tension. It also defines boiling point, melting point, viscosity, and vapor pressure in relation to the strength of intermolecular forces.
8. LONDON DISPERSION FORCES
-is the weakest intermolecular force. The
London dispersion force is a temporary
attractive force that results when the electrons
in two adjacent atoms occupy positions that
make the atoms form temporary dipoles. This
force is sometimes called an induced dipole-
induced dipole attraction.
9.
10. Dipole-Dipole Forces
- attractive forces between the positive end of one polar
molecule and the negative end of another polar
molecule.
15. Hydrogen bonding
-is a special type of dipole-dipole attraction between
molecules, not a covalent bond to a hydrogen atom.
It results from the attractive force between a
hydrogen atom covalently bonded to a very
electronegative atom such as a N, O, or F atom and
another very electronegative atom.
16.
17. Boiling Point- is the temperature at which the
vapour pressure of a liquid is equal to the
external pressure.
18. Melting Point- is the temperature at which
a substance begins to change from solid to
liquid.
19. Viscosity- is the property of substance resistance to flow, In
general, stronger IMF means high viscosity.
20. Vapor pressure- is a measure of the tendency of a material
to change into the gaseous or vapor state.
